Balancing Net Ionic Equations

This video tutorial guides viewers through balancing the net ionic equation for barium chlorate and sodium phosphate. It begins with balancing the molecular equation, followed by determining the states of substances based on solubility rules. The tutorial then explains how to split strong electrolytes into ions for the complete ionic equation and identifies spectator ions. Finally, it presents the balanced net ionic equation, ensuring charge conservation and atom balance.

What is the first step in balancing a net ionic equation?

• Write the net ionic equation

• Determine the solubility of compounds

• Balance the molecular equation

• Identify the spectator ions

How many barium atoms are needed to balance the molecular equation?

• One

• Four

• Two

• Three

Which of the following compounds is generally insoluble?

• Barium phosphate

• Ammonium sulfate

• Sodium chloride

• Potassium nitrate

What happens to the precipitate in a chemical reaction?

• It dissolves in the solution

• It forms a gas

• It reacts with the solvent

• It falls to the bottom of the test tube

What is the role of spectator ions in a chemical reaction?

• They remain unchanged and do not participate

• They change the color of the solution

• They form a precipitate

• They participate in the reaction

Which ions are considered spectator ions in the given reaction?

• Barium ions

• Chlorate ions

• Phosphate ions

• Hydrogen ions

What must be conserved in a balanced net ionic equation?

• Mass only

• Charge only

• Both mass and charge

• Neither mass nor charge

How is the net charge of the reactants and products related in a balanced equation?

• Reactants have a higher charge

• Charge is not considered

• Products have a higher charge

• Both have the same net charge

What is the net charge of the balanced net ionic equation in this video?

• Positive

• Negative

• Variable

• Zero

What is the final step in writing a net ionic equation?

• Ensuring charge conservation

• Balancing the atoms

• Writing the molecular equation

• Identifying the precipitate